mccord ch301

exam 1

9/17


Where do I go for my Exam 1 ?

Monday • 9/17 • 7:30 - 9pm


9:30 Class

Room Assignments:

last names A - Mi in BUR 106

last names Mo - Z in JES A121A

Please make SURE you go to the right room!

11:00 Class

Room Assignments:

last names A - Mi in UTC 2.112A

last names Mo - Z in UTC 2.102A

Please make SURE you go to the right room!

What we provide on Exams We will provide all students with:

  • copy of the exam
  • an answer sheet - aka: bubblesheet
  • a Periodic Table Handout sheet
  • scratch paper if needed

Note that the periodic table handout is available on the gchem site in the appendix under "Exam Preparation". Here is a direct link to the Periodic Table Handout for Exam 1.

Coverage: Exam 1 covers all the material that was covered on LE's 01-09 and HW01, HW02, and HW03. Most of the exam is over Chapter 2 (Gases) from the gchem site. There will be about 3 questions that are "fundamentals" (Chapter 1) which means you would be balancing and equation and calculating stoichiometric quantities (especially gases). Know that this exam is really about gases.

Questions: The exam will be have 20 multiple choice questions. The questions will have an equal weight of 5 points each. Point values are included with all questions. We will only grade you by what is bubbled in on the answer sheet. We will not look at your exam copy for answers, nor consider them in any way. Bubble carefully and correctly.

Bring the Following to the Exam

  • a pencil(s) - mechanical or wood
  • scanner only reads pencil - no ink!
  • bring eraser if you are prone to mistakes
  • bring a non-programmable, non-graphing, scientific calculator
  • we provide the rest - see top of page

DO NOT bring...

  • ink pens
  • graphing calculator
  • any type of programmable calculator
  • electronic devices - including earbuds, etc...
  • smart watches - put away that Apple Watch!
  • small creatures - or large... no creatures

Main Equations/Formulas for Exam 1

Ideal Gas Law: \[PV = nRT\]

Dalton's Law of Partial Pressures: \[P_{\rm total}= P_{\rm A} + P_{\rm B} + P_{\rm C} + \cdots \]

Kinetic Energy of an Ideal Gas: \[E_{\rm k} = {3\over 2} RT\]

Root Mean Squared Speed of particles: \[v_{\rm rms} = \sqrt{3RT\over M}\]

Van der Waal's Equation of State
\[\left(P+a{n^2 \over V^2}\right)(V-nb)=nRT\]

Learning Outcomes for Gases

Students will be able to...

  1. Describe pressure from a macroscopic and microscopic perspective.
  2. Relate Boyles, Charles', and Avogadro's gas laws to observations of gas behavior.
  3. Calculate the values for state functions (n, V, T, P) using the ideal gas equation.
  4. Define the conditions of STP and SATP.
  5. Relate the number density and mass density for a given gas, including quantitative calculations such as mass, molecular weight, and density.
  6. Relate partial pressures and the total pressure as described by Dalton’s Law of Partial Pressure.
  7. Apply the concept of the gas laws to gas phase reactions.
  8. Perform stoichiometric calculations using gas properties, masses, moles, limiting reagents, and percent yield.
  9. Relate kinetic energy to the temperature of a gas.
  10. Relate temperature, molar mass, and gas velocity.
  11. Describe the effect of molar mass and temperature on the Maxwell-Boltzmann gas velocity distribution.
  12. Apply kinetic molecular theory to a variety of gas phenomena including diffusion and effusion.
  13. Calculate relative effusion and diffusion rates using Graham’s Law.
  14. Explain the quantitative relationship between state functions (n, T, V, and P) as described by kinetic molecular theory.
  15. Describe macroscopic gas behavior using a small particle model of a gas.
  16. State when the ideal gas model fails to predict the behavior of gases observed in nature and in the laboratory.
  17. Explain what the breakdown of the ideal gas law reveals about the assumptions of kinetic molecular theory.
  18. Explain the general principles of the hard sphere model and van der Waal's model of gas.